2.) The following wavelengths are found among the many radiations emitted by sin

Question

2.) The following wavelengths are found among the many radiations emitted by singly ionized helium: 24.30 nm, 25.63 nm, 102.5 nm, 320.4 nm. If we group the transitions in helium as we did in hydrogen by identyfying the final state no and initial state n, to which series does each transition belong?

I am familiar with the fact that I need to use the formula for wavelengths given by Rydbergs constant, however I am unsure if I need to solve for each series with a new quantum value for the Rydberg constant.

Do I need to do this? Or can I follow the bohr model because ionized helium only has one electron such as hydrogen does.

Please lend some help if you are knowledgable on this subject. Your efforts will be rewarded and greatly appreciated!

Explanation / Answer

Since you already know about the working out part, i'll simply answer your doubt.

Please note that you have to calculate it for each one by substituting the given values. This is needed because even though there is only one electron like in Hydrogen, the value of Z(the nuclear charge) will be different for Helium and Hydrogen. The value of Z is 2 foe He+ and 1 for H. So we cannot follow the same Bohr's model as we did for Hydrogen. We have to do it independently and then group the respective transitions.

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